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Percent I new 1. Balanced the equation for this reaction, and answer the questions. C(s) + H₂O (g) → CH₁ (g) + CO₂ (g) How many grams of methane, CH4, can be produced from 235.0 g carbon reacted in an excess of water? a) 1 - b) If 126.0 g CH4 are actually collected in the lab, what is the percent yield?

Percent I new 1. Balanced the equation for this reaction, and answer the questions. C(s) + H₂O (g) → CH₁ (g) + CO₂ (g) How many grams of methane, CH4, can be produced from 235.0 g carbon reacted in an excess of water? a) 1 - b) If 126.0 g CH4 are actually collected in the lab, what is the percent yield?

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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1. Balanced the equation for this reaction, and answer the questions. H₂O (g) → CH4 (g) + _____ CO₂ (g) C(s) + How many grams of methane, CH4, can be produced from 235.0 g carbon reacted in an excess of water? a) b) If 126.0 g CH4 are actually collected in the lab, what is the percent yield? 2. The oxidation of ammonia, NH3, is represented in the following equation. Balance the equation and answer the questions. NH3 + O2 → NO +_______ H₂O a) How many grams of water can be formed when 37.5 g NH3 reacts with an excess of oxygen? b) When this reaction is run, 57.75 g H₂O is produced. What is the percent yield for this result? 3. A reaction yields 8.77 g of a product. What is the percent yield if the theoretical yield is 14.80 g? 4. Balance the equation and answer the question. Be + HCI → HCI →→_____ BeCl₂ + H₂ The mass of beryllium chloride produced produced in the lab was 18.95 g. What is the percent yield if this reaction was run with 2.45 g beryllium in an excess of HCI?
Transcribed Image Text:1. Balanced the equation for this reaction, and answer the questions. H₂O (g) → CH4 (g) + _____ CO₂ (g) C(s) + How many grams of methane, CH4, can be produced from 235.0 g carbon reacted in an excess of water? a) b) If 126.0 g CH4 are actually collected in the lab, what is the percent yield? 2. The oxidation of ammonia, NH3, is represented in the following equation. Balance the equation and answer the questions. NH3 + O2 → NO +_______ H₂O a) How many grams of water can be formed when 37.5 g NH3 reacts with an excess of oxygen? b) When this reaction is run, 57.75 g H₂O is produced. What is the percent yield for this result? 3. A reaction yields 8.77 g of a product. What is the percent yield if the theoretical yield is 14.80 g? 4. Balance the equation and answer the question. Be + HCI → HCI →→_____ BeCl₂ + H₂ The mass of beryllium chloride produced produced in the lab was 18.95 g. What is the percent yield if this reaction was run with 2.45 g beryllium in an excess of HCI?
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